Refer to Example 14-1. How many grams of CH₃CH₂OH must be added to 100.0 mL of the solution described in part (d) to increase the mole fraction of CH₃CH₂OH to 0.0525?

Example 14-1

An ethanol–water solution is prepared by dissolving 10.00 mL of ethanol, CH₃CH₂OH (d = 0.789 g/mL), in a sufficient volume of water to produce 100.0 mL of a solution with a density of 0.982 g/mL(Fig. 14-1). What is the concentration of ethanol in this solution expressed as 

(a) Volume percent; 

(b) Mass percent; 

(c) Mass/volume percent; 

(d) Mole fraction; 

(e) Mole percent;

(f) Molarity; 

(g) Molality?

Figure 14-1

Transcribed Image Text:

Water 10.00 mL CH3CH₂OH Volumetric flask 100.0 mL→ Ethanol-water solution: d = 0.982 g/mL